The reaction between nitrogen dioxide and carbon monoxide is NO₂(g) + CO(g) → NO(g) + CO₂(g) The rate constant at 701 K is measured as 2.57 M-1.s and that at 895 K is measured as 567 M-1.8-¹. Part A Use the value of the activation energy (E₁ = 1.50 x 10² kJ/mol) and the given rate constant of the reaction at either of the two temperatures to predict the rate constant at 459 K. 1957 ΑΣΦ xa x₁ = √x √x x x x x.10 k= 3.32 10-4 ● Submit Previous Answers Request Answer X Incorrect; Try Again; 2 attempts remaining SWIX ? SAI M-1.8-1

The reaction between nitrogen dioxide and carbon monoxide is NO₂(g) + CO(g) → NO(g) + CO₂(g) The rate constant at 701 K is measured as 2.57 M-1.s and that at 895 K is measured as 567 M-1.8-¹. Part A Use the value of the activation energy (E₁ = 1.50 x 10² kJ/mol) and the given rate constant of the reaction at either of the two temperatures to predict the rate constant at 459 K. 1957 ΑΣΦ xa x₁ = √x √x x x x x.10 k= 3.32 10-4 ● Submit Previous Answers Request Answer X Incorrect; Try Again; 2 attempts remaining SWIX ? SAI M-1.8-1

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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a)The activation energy of a certain reaction is 48.9 kJ/mol. At 27 ∘C , the rate constant is 0.0160s ^−1 . At what temperature in degrees Celsius would this reaction go twice as fast? Express your answer with the appropriate units. b)Given that the initial rate constant is 0.0160s ^−1at an initial temperature of 27 ∘C , what would the rate constant be at a temperature of 200. ∘C for the same reaction described in Part A? Express your answer with the appropriate units.
The activation energy for a particular reaction is 102 kJ/mol. If the rate constant is 1.35 × 10⁻⁴ s⁻¹ at 305 K, what is the rate constant at 273 K?
The decomposition of hydrogen iodide on a gold surface at 150 °C HI(g) 2 H2(g) + ½ I2(g) is zero order in HI with a rate constant of 1.20x10-4 M s1. If the initial concentration of HI is 0.376 M, the concentration of HI will be | M after 2.74x103 seconds have passed.
For the reaction: NO2(g) → 1/2 O2(g) + NO (g) The following data were obtained: Time (s) 0 50 100 [NO₂] (M) 0.01 Concentration NO2 0.00787 -4.844697217 127.064803 200 0.00481 -5.337058195 0.00649 -5.037492748 154.0832049 300 0.0038 -5.572754212 0.012 0.01 0.008 Natural Log [NO2] (M) Determine the rate law of this reaction and the value of k, the rate constant. The graphs of the data appear below. 0.006 0.004 -4.605170186 100 0.002 0 0 1/[NO2] 100 200 Time (s) 207.9002079 1/[NO2] 263.1578947 y = -1.97E-05x + 9.15E-03 R² = 9.27E-01 300 250 200 150 100 50 0 300 0 50 400 100 Natural Log [NO2] 150 -4.5 -4.7 -4.9 -5.1 -5.3 -5.5 -5.7 0 200 Time (s) y = 0.5431x + 99.833 R² = 1 100 250 300 200 Time (s) 350 y = -0.0032x - 4.6679 R² = 0.9824 300 400
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For the gas phase decomposition of isobutyl bromide, (CH3),CHCH,Br–→{CH3),C=CH, + HBr the rate constant at 639 K is 6.60×105 /s and the rate constant at 682 K is 8.07x104 /s. The activation energy for the gas phase decomposition of isobutyl bromide is kJ.
The first order reaction SO,CI, (g) --> SO2 (g) + Cl2 (g) has a rate constant of 2.90 X 10 s at a given temperature. Determine that concentration of SO,Cl, at 1,621 s if the initial concentration of SO,Cl, is 0.101 M.
Consider following reaction: 2 A2B5(g) → 4AB2(g) + B2(g) The rate constant is 0.129 s-1 at 298 K for this reaction. What is the percent of A2B5 left after the first 19.091 s? Report your answer with three decimals. Enter numbers only;
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The rate constant of a first-order reaction is 4.60 x 10* s at 350 degrees Celsius. If the activation energy is 104 kJ/mol, calculate the temperature at which its rate constantis 8.80 x 104 s?.
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